[Review Topics] [References] One cubic meter of methane hydrate has 164 m of CH, (at STP). If you burn the methane in 8.50 m of hydrate [to give CO2 (g) and H20(g)], how much energy, as heat, can be obtained? Species AƒH, kJ/mol CH4 (g) -74.87 02(g) 0. CO2(g) -393.509 H2O(g) -241.83 Energy obtained kJ %3D Submit Answer Retry Entire Group 4 more group aftempts remaining 10:11 PM FLU 3/21/2020

[Review Topics] [References] One cubic meter of methane hydrate has 164 m of CH, (at STP). If you burn the methane in 8.50 m of hydrate [to give CO2 (g) and H20(g)], how much energy, as heat, can be obtained? Species AƒH, kJ/mol CH4 (g) -74.87 02(g) 0. CO2(g) -393.509 H2O(g) -241.83 Energy obtained kJ %3D Submit Answer Retry Entire Group 4 more group aftempts remaining 10:11 PM FLU 3/21/2020

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 81E: Among the substances that react with oxygen and that have been considered as potential rocket fuels...

See similar textbooks

Similar questions

The combustion of 0.4196 g of a hydrocarbonreleases 17.55 kJ of heat. The masses of theproducts are ??2 = 1.419 g and ?2? = 0.290 g.a. If the approximate molar mass of thecompound is 76 g, calculate its standardenthalpy of formation.
Ethylene (C₂H₄) is the starting material for the preparationof polyethylene. Although typically made during the processingof petroleum, ethylene occurs naturally as a fruit-ripening hor-mone and as a component of natural gas. (a) The heat of reactionfor the combustion of C₂H₄ is 1411 kJ/mol. Write a balancedthermochemical equation for the combustion of C₂H₄. (b) Howmany grams of C₂H₄ must burn to give 70.0 kJ of heat?
Compound X and Y are being tested for their capacity as insulators. a. In the first experiment, compound X after being heated to 200 F it was transferred to a 0.100L water bath, the initial temperature of the water bath is 25 C, the final temperature after compound X was dropped was 30 C. What is the specific heat in calories? (specific heat of water is 1 calorie/gram °C = 4.186 joule/gram °C) b. The same experiment was conducted with chemical Y but the final temperature of the water bath was 308 K. What is the specific heat in Joules? c. Which of the two chemicals would be a better insulator? and Why?
Calculate the heat energy (ΔHreaction) produced when 1 mole of ethanol burns to produce CO2 and H2O as given below: C2H5OH (l) + 3O2 (g) → 2CO2 (g) + 3H2O (l)
Given the following, how much heat is evolved when 0.025 m3 of CH6N2 is combusted at STP?
Calculate the heat energy (ΔHreaction) produced when 1 mole of ethanol burns to produce CO2 and H2O C2H5H(l) + 3O2 (g) ---> 2CO2 (g) +3H2O (l)
Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat produced by combustion of one mole of acetylene in such a torch is likely not equal to the enthalpy of combustion of acetylene listed in Table 5.2. Considering the conditions for which the tabulated data are reported, suggest an explanation.
Among the substances that react with oxygen and that have been considered as potential rocket fuels are diborane [ B2H6, produces B2O3(s) and H2O(g) ], methane [ CH4, produces CO2(g) and H2O(g) ], and hydrazine [ N2H2, produces N2(g) and H2O(g) ]. On the basis of the heat released by 1.00 g of each substance in its reaction with oxygen, which of these compounds offers the best possibility as a rocket fuel? The Hf of B2H6(g), CH4(g), and N2H4(l) may be found in Appendix G.
Calculate the enthalpy change when 1.0(1 g of methane is burned in excess oxygen according to the reaction CH,(g) 4- 2O2(g) ->CO2(g) + H-CH/) 1H = -891 kJ/mol
9.56 Using heats of formation tabulated in Appendix E, calculate the heats of reaction for the following. (a) C2H2(g)+52O2(g)2CO2(g)+H2O(l) (b) PCl3(g)+Cl2(g)PCl5(g) (c) C2H4(g)+H2O(g)C2H5OH(g) (d) Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(l)
Give only typing answer with explanation and conclusion to all parts CH4 + 2O2 ------- CO2 + 2H2O + 890.1 kj What is theoretical yield of CO2 in moles using 1.5 moles of O2? What is theoretical yield of H2O in grams using 1.5 moles of CH4? How much heat is released by burning 120 g of O2?
C2H5OH combustion releases 1200 kJ/mol. How many giving off of C2H5OH is to be burned to generate 6200 kJ energy?